Electrochemistry - Live Session

Which of the following solutions has the highest equivalent conductance?
(1) 0.01 M NaCl
(2) 0.05 M NaCl
(3) 0.005 M NaCl
(4) 0.02 M NaCl

The resistance of 0.01 N solution of an electrolyte AB at 328K is 100 ohm. The specific conductance of solution is
(cell constant = 1 $c m^{- 1}$ )
(1) 100 ohm
(2) $10^{- 2}$ ohm
(3) $10^{- 2} o h m^{- 1} c m^{- 1}$
(4) $10^{2}$ ohm-cm

The increase in the molar conductivity of HCI with dilution is due to
1. Increase in the self ionisation of water
2. Hydrolysis of HCI
3. Decrease in the self ionisation of water
4. Decrease in the interionic forces

A solution of $N a_{2} S O_{4}$ in water is electrolysed using pt electrodes. The products at the cathode and anod are respectively
(1) $H_{2}, S O_{2}$
(2) $O_{2}, N a O H$
(3) $H_{2}, O_{2}$
(4) $O_{2}, S O_{2}$

Given that
$A g^{+} / A g \to + 0.80 V$ $C o^{2 +} / C o \to - 0.28 V$
$C u^{2 +} / C u \to + 0.34 V$ $Z n^{2 +} / Z n \to - 0.76 v$
The most reactive metal which displaces other metals from their salts in solution is
(1) Ag
(2) Cu
(3) Co
(4) Zn

The emf of the cell
TI | TI $^{+}$ (0.001 M) || Cu $^{2 +}$ (1M) | Cu is 0.83 V. The emf of this cell could be increased by
(1) Increasing in the concentration of TI $^{+}$ ions
(2) Increasing in the concentration of Cu $^{+}$ ions
(3) Increasing in the concentration of both
(4) None of the above

For a reaction A(s) + 2 $B^{+} \leftrightarrow A^{2 +} + 2 B (s); K_{c}$ has been found to be 10¹². The E $°$ cell is-
1. 0.354 V
2. 0.708 V
3. 0.0098V
4. 1.36V
.

The solutions of nickel sulphate in which nicked rod dipped is diluted to 10 times. The
potential of nickel
(1) Decreases by 60 mV
(2) Increases by 30 mV
(3) Decreases by 30 mV
(4) Decreases by 60 mV

Two electrodes are fitted in conductance cell 1.5 cm apart while the area of cross-section
of 1.5 cm apart while the area of cross-section of each electrode is 0.75 cm². The cell
constant is-
1. 1.0125 cm
2. 0.5 cm
3. 2.0 cm^-1
4. 0.2cm^-1

10.

Pick out the incorrect statement
1. Equivalent conductance increase with dilution
2. Molar conductance increase with dilution
3. Specific conductance increase with dilution
4. Specific resistance increase with dilution

11.

The value of $\land$ $_{e q}^{\infty}$ for NH₄Cl, NaOH and NaCl are respectively 149.74, 248.1 and 126.4 ${ohm}^{- 1} {cm}^{2} {equiv}^{- 1} .$ The value of $\land$ $_{e q}^{\infty}$ of NH₄OH is -
1. 317.44
2. 271.44
3. 71.44
4. It cannot be calculated from the data given

12.

In passing 3 faradays of electricity through the three electrolytic cells connected in
series containing $A g^{+}, C u^{2 +} a n d A l^{3 +}$ respectively. The molar ratio in which the three
metal ions are liberated at the electrode is
(1) 1 :2 :3
(2) 3 :2 :1
(3) 6:3 : 2
(4) 3 :4 : 2

13.

During electrolysis of fused calcium hydride , the hydrogen is produced at
(1) Cathode
(2) Anode
(3) Hydrogen is not liberated at all
(4) H $_{2}$ produced reacts with oxygen to form water

14.

The current liberates 0.504 g of hydrogen in 2 hours, the amount of copper liberated
from a solution of CuSO $_{4}$ by the same current flowing for the same time would be
(1) 31.8g
(2) 63.6g
(3) 15.9 g
(4) 6.36g

15.

Given that
$I_{2} + 2 e \to 2 \bar{I;}$ E⁰ = 0.54V
Br 2 + $2 \bar{e}$ $\to 2 B r; E^{0} = 1.09 V$
Predict which of the following is true
(1) $\bar{I}$ Ions will be able to reduce bromine
(2) $\bar{B r}$ ion will be to able to reduce iodine
Indine will be able to reduce bromine inos
Bromise will be able to reduce iodide ions

16.

The potential of hydrogen electrode having a pH = 10 is
1. 0.59V
2. -0.59V
3. 0V
4. -59V

17.

The EMF of the given cell is-
Zn(s) $|Z n^{+ 2}|$ (0.1M) $||||$ Sn⁺² (0.001M) $|S n (s)|$
Given E⁰_Zn²⁺_/Zn =-0.76v, E⁰_Sn²⁺_/Sn =-0.14V
1. 0.62V
2. 0.56V
3. 1.12V
4. 0.31V

18.

Zinc gives H₂ with H₂SO₄ and HCI but not with HNO₃ because
(1) Zinc acts as oxidizing agent when react with HNO₃
(2) HNO 3 is a weaker acid then H₂SO₄ and HCI
(3) In electrochemical series, the zine is above hydrogen
(4) NO $\bar{3}$ is reduced is a preference to hydronium ion

19.

An aqueous solution containing one mole per litre of each
$Cu {({NO}_{3})}_{2}, Ag {({NO}_{3})}_{2}, Mg {({NO}_{3})}_{2}$ is
being electrolysed using inert electrodes. The values of standard electrode potential in volts (reduction potential) are
$Ag |{Ag}^{+} = + 0.80 2 Hg| {Hg}^{2 +} = + 0.79$
${Cu}^{2 +} / C u = + 0.34 {Mg}^{2 +} / Mg = - 2.37$ is
(1) Ag,Hg,Cu,Mg
(2) Mg,Cu,Hg,Ag
(3) Ag,Hg,Cu
(4) Cu,Hg,Ag

20.

Standard electrode potential data are useful for understanding the suitability of an oxidant in aredox titration. Some half cell reactions and their standard potential are given below

${MnO}_{4}^{-} (aq) + 8 H^{+} (aq) + 5 e^{-} \to {Mn}^{2 +} (aq) + 4 H_{2} O (l); E ° = 1.51 V$
${Cr}_{2} O_{7} {}_{2 -}(aq) + 14 H^{+} (aq) + 6 e^{-} \to 2 {Cr}^{3 +} (aq) + 7 H_{2} O (l); E ° = 1.38 V$

{Fe}^{3 +} (aq) + e^{-} \to {Fe}^{2 +} (aq); E ° = 0.77 V

${Cl}_{2} (g) + 2 e^{-} \to 2 {Cl}^{-} (aq); E ° = 1.40 V$
Identify the only incorrect statement regarding the quantitative estimation of aqueous $Fe (NO$
${MnO}_{4}^{-}$ can be used in aqueous $HCl$
${Cr}_{2} O_{7}^{2 -}$ can be used in aqueous $HCl$
${MnO}_{4}^{2 -}$ can be used in aqueous $H_{2} {SO}_{4}$
${Cr}_{2} O_{7}^{2 -}$ can be used in aqueous $H_{2} {SO}_{4}$

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